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Chapter 14: Problem 113

Given that the \(K_{\mathrm{a}}\) value for acetic acid is \(1.8 \times 10^{-5}\) and the \(K_{\mathrm{a}}\) value for hypochlorous acid is \(3.5 \times 10^{-8}\), which is the stronger base, \(\mathrm{OCl}^{-}\) or \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}\) ?

Short Answer

Expert verified
The stronger base is \(\mathrm{OCl}^{-}\) (hypochlorite ion), as its conjugate acid, Hypochlorous Acid (\(\mathrm{HOCl}\)), has a lower \(K_{\mathrm{a}}\) value compared to Acetic Acid (\(\mathrm{CH}_{3}\mathrm{COOH}\)).

Step by step solution

01

Write down the given values

The given \(K_{\mathrm{a}}\) values are: Acetic Acid (\(\mathrm{CH}_{3}\mathrm{COOH}\)): \(K_{\mathrm{a}} = 1.8 \times 10^{-5}\) Hypochlorous Acid (\(\mathrm{HOCl}\)): \(K_{\mathrm{a}} = 3.5 \times 10^{-8}\)
02

Compare the \(K_{\mathrm{a}}\) values

By comparing the \(K_{\mathrm{a}}\) values, we see that: \(K_{\mathrm{a}}\) for Acetic Acid (\(\mathrm{CH}_{3}\mathrm{COOH}\)) > \(K_{\mathrm{a}}\) for Hypochlorous Acid (\(\mathrm{HOCl}\)), i.e., \(1.8 \times 10^{-5} > 3.5 \times 10^{-8}\)
03

Determine the stronger acid and weaker base

Since Acetic Acid has a higher \(K_{\mathrm{a}}\) value, it's a stronger acid than Hypochlorous Acid. As a result, its conjugate base, \(\mathrm{C}_{2}\mathrm{H}_{3}\mathrm{O}_{2}^{-}\) (acetate ion), is weaker than \(\mathrm{OCl}^{-}\) (hypochlorite ion).
04

Conclude which is the stronger base

Based on the comparison made in Step 3, we determine that \(\mathrm{OCl}^{-}\) (hypochlorite ion) is the stronger base compared to \(\mathrm{C}_{2}\mathrm{H}_{3}\mathrm{O}_{2}^{-}\) (acetate ion).

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Most popular questions from this chapter

Hemoglobin (abbreviated \(\mathrm{Hb}\) ) is a protein that is responsible for the transport of oxygen in the blood of mammals. Each hemoglobin molecule contains four iron atoms that are the binding sites for \(\mathrm{O}_{2}\) molecules. The oxygen binding is pH-dependent. The relevant equilibrium reaction is $$\mathrm{HbH}_{4}^{4+}(a q)+4 \mathrm{O}_{2}(g) \rightleftharpoons \mathrm{Hb}\left(\mathrm{O}_{2}\right)_{4}(a q)+4 \mathrm{H}^{+}(a q)$$ Use Le Châtelier's principle to answer the following. a. What form of hemoglobin, \(\mathrm{HbH}_{4}{ }^{4+}\) or \(\mathrm{Hb}\left(\mathrm{O}_{2}\right)_{4}\), is favored in the lungs? What form is favored in the cells? b. When a person hyperventilates, the concentration of \(\mathrm{CO}_{2}\) in the blood is decreased. How does this affect the oxygenbinding equilibrium? How does breathing into a paper bag help to counteract this effect? (See Exercise 148.) c. When a person has suffered a cardiac arrest, injection of a sodium bicarbonate solution is given. Why is this necessary?

Trichloroacetic acid \(\left(\mathrm{CCl}_{3} \mathrm{CO}_{2} \mathrm{H}\right)\) is a corrosive acid that is used to precipitate proteins. The \(\mathrm{pH}\) of a \(0.050 \mathrm{M}\) solution of trichloroacetic acid is the same as the \(\mathrm{pH}\) of a \(0.040 \mathrm{M} \mathrm{HClO}_{4}\) solution. Calculate \(K_{\mathrm{a}}\) for trichloroacetic acid.

Write the reaction and the corresponding \(K_{\mathrm{b}}\) equilibrium expression for each of the following substances acting as bases in water. a. aniline, \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\) b. dimethylamine, \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NH}\)

Identify the Lewis acid and the Lewis base in each of the following reactions. a. \(\mathrm{Fe}^{3+}(a q)+6 \mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}(a q)\) b. \(\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CN}^{-}(a q) \rightleftharpoons \mathrm{HCN}(a q)+\mathrm{OH}^{-}(a q)\) c. \(\mathrm{HgI}_{2}(s)+2 \mathrm{I}^{-}(a q) \rightleftharpoons \mathrm{HgI}_{4}{ }^{2-}(a q)\)

Calculate the \(\mathrm{pH}\) of a \(0.10 \mathrm{M} \mathrm{CoCl}_{3}\) solution. The \(K_{\mathrm{a}}\) value for \(\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}\) is \(1.0 \times 10^{-5}\).
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